Textbook-Integrated Guide to Educational Resources

TIGER

Data Pooling in a Chemical Kinetics Experiment: The Aquation of a Series of Cobalt(III) ComplexesRichard S. Herrick, Kenneth V. Mills, and Lisa P. NestorDescribes an experiment that introduces students to integrated rate laws, the search for a mechanism that is consistent with chemical and kinetic data, and the concept of activation barriers and their measurement in a curriculum whose pedagogical philosophy makes the laboratory the center of learning for undergraduates in their first two years of instruction.Herrick, Richard S.; Mills, Kenneth V.; Nestor, Lisa P. J. Chem. Educ.2008, 85, 1120.

Coordination Compounds |

Kinetics |

Mechanisms of Reactions |

Rate Law |

UV-Vis Spectroscopy

Reaction Order Ambiguity in Integrated Rate PlotsJoe LeeThis article provides a theoretical and statistical justification for the necessity of monitoring a reaction to a substantial fraction of completion if integrated rate plots plots are to yield unambiguous orders.Lee, Joe. J. Chem. Educ.2008, 85, 141.

The Chemistry of Paper PreservationHenry A. CarterThis article examines the applications of chemistry to paper preservation. The acid-catalyzed hydrolysis of cellulose accounts for the deterioration of paper in library books and other written records. To combat this threat to our written heritage, new permanent papers have been developed that are relatively chemically stable and undergo a very slow rate of deterioration. Carter, Henry A. J. Chem. Educ.2007, 84, 1937.

Acids / Bases |

Applications of Chemistry |

Aqueous Solution Chemistry |

Free Radicals |

Gas Chromatography |

HPLC |

pH |

Kinetics |

Rate Law

How Many Atomic Layers of Zinc Are in a Galvanized Iron Coating? Shui-Ping YangThis article describes a guided inquiry and problem solving experiment in which students use a novel gasometric assembly to determine the thickness and number of atomic layers of zinc coating on galvanized iron wires and nails.Yang, Shui-Ping. J. Chem. Educ.2007, 84, 1792.

Aqueous Solution Chemistry |

Consumer Chemistry |

Electrochemistry |

Gases |

Laboratory Equipment / Apparatus |

Quantitative Analysis |

Rate Law

Visualizing the Transition State: A Hands-on Approach to the Arrhenius EquationThomas S. Kuntzleman, Matthew S. Swanson, and Deborah K. SayersPennies and dice are used to simulate the kinetics of two irreversible "reactions" with a hands-on, Monte Carlo approach. Arrhenius plots of the data generated yield activation energies comparable to assigned values and pre-exponential factors close to what would be expected based on the probability of a "reactant" achieving the correct orientation for conversion into "product". A comparison of the values obtained for the pre-exponential factors for the different simulations allows students to semi-quantitatively discuss the orientational requirement that is contained within this factor.Kuntzleman, Thomas S.; Swanson, Matthew S.; Sayers, Deborah K. J. Chem. Educ.2007, 84, 1776.

Kinetics |

Rate Law

A Student Laboratory Experiment Based on the Vitamin C Clock ReactionEd VitzDescribes an adaptation of the vitamin C clock reaction to a student laboratory experiment in which the orders with respect to peroxide and iodide, the rate constant, and the activation energy are determined by the method of initial rates.Vitz, Ed. J. Chem. Educ.2007, 84, 1156.

Consumer Chemistry |

Kinetics |

Mechanisms of Reactions |

Rate Law

An Inexpensive Kinetic Study: The Reaction of FD&C Red #3 (Erythrosin B) with HypochloriteMaher M. Henary and Arlene A. RussellStudents use a desktop visible spectrophotometer to quantitatively follow the rate of disappearance of FD&C Red #3 with hypochlorite. The first-order reaction in both dye and bleach yields simple data that students can easily process and graph using spreadsheet software to obtain the rate constant and the rate law.Henary, Maher M.; Russell, Arlene A. J. Chem. Educ.2007, 84, 480.

Dyes / Pigments |

Kinetics |

Rate Law |

UV-Vis Spectroscopy

Applications of Reaction RateKevin CunninghamThis article presents an assignment in which students are to research and report on a chemical reaction whose increased or decreased rate is of practical importance. The assignment is designed to develop and assess a number of valuable skills and understandings, including the ability to write effectively.Cunningham, Kevin. J. Chem. Educ.2007, 84, 430.

Textbook Deficiencies: Ambiguities in Chemical Kinetics Rates and Rate ConstantsKeith T. Quisenberry and Joel TellinghuisenRecommends that textbook authors make it clear that (i) the reaction rate and rate constant cannot be defined unambiguously without explicitly stating the reaction for which they apply and therefore (ii) the relation between the half-life, which is a physical property of the reaction system, and the rate constant depends upon how the reaction is written.Quisenberry, Keith T.; Tellinghuisen, Joel. J. Chem. Educ.2006, 83, 510.

Steel Wool and Oxygen: How Constant Should a Rate Constant Be?Michiel VogelezangIn the article Steel Wool and Oxygen: A Look at Kinetics, James Gordon and Katherine Chancey describe an experiment about the kinetics between iron and oxygen. Like all good experiments this one is easy to carry out and produces good results. However, the experiment can even have a greater impact with only a small addition.Vogelezang, Michiel. J. Chem. Educ.2006, 83, 214.

Rate Law |

Kinetics |

Oxidation / Reduction

Robust Linear Regression Using Theil's MethodP. GlaisterThe method of least squares is not resistant to the undue influence outliers can have on the estimate of slope and intercept. An alternative approach is to use a method that is specifically designed to reduce the effect that outliers can have on slope and intercept estimates.Glaister, P. J. Chem. Educ.2005, 82, 1472.

Factors Affecting Reaction Kinetics of Glucose OxidaseKristin A. JohnsonDemonstration based on a biochemical kinetics experiment in which the rate of reaction varies with the enzyme concentration, substrate concentration, substrate used in the reaction, and temperature. Johnson, Kristin A. J. Chem. Educ.2002, 79, 74.

Combustion Demonstration Using Updated Flame TornadoEdward G. SenkbeilThis demonstration uses the combustion of different forms of cellulose and an updated version of the "flame tornado" as an ignition source to illustrate the factors affecting the combustion process. The objectives of the experiment are to illustrate the factors affecting the rate of a combustion reaction and to demonstrate the factors affecting the production of a flame by using the flame tornado. Senkbeil, Edward G. J. Chem. Educ.2000, 77, 1449.

Descriptive Chemistry |

Oxidation / Reduction |

Reactions |

Rate Law

Simulating Dynamic Equilibria: A Class ExperimentJohn A. Harrison and Paul D. BuckleyA first-order reversible reaction is simulated on an overhead projector using small coins or discs. Results illustrate how dynamic equilibria are established and allow the introduction of the concept of an equilibrium constant. Le Chtelier's principle is illustrated by further simulations. Harrison, John A.; Buckley, Paul D. J. Chem. Educ.2000, 77, 1013.

Equilibrium |

Rate Law |

Reactions

Chemistry and Flatulence: An Introductory Enzyme ExperimentJohn R. Hardee, Tina M. Montgomery, and Wray H. JonesAn enzyme experiment using raffinose family sugars extracted from green split peas as a substrate and the enzymes alpha-galactosidase and sucrase found in Beano. The reaction studied was the hydrolysis of raffinose family sugars to galactose, glucose, and fructose, and the reaction rate was determined using a retail glucometer to measure the concentration of glucose.Hardee, John R.; Montgomery, Tina M.; Jones, Wray H. J. Chem. Educ.2000, 77, 498.

Nonmajor Courses |

Enzymes |

Food Science |

Rate Law |

Catalysis |

Applications of Chemistry

An Experiment to Demonstrate How a Catalyst Affects the Rate of a ReactionChristine L. Copper and Edward KoubekThis experiment, which is a modified version of the traditional iodine clock reaction, allows students to calculate rates of reaction, orders of reactants, and activation energies. It also lets students discover that to increase a reaction's rate, a catalyst need only provide any additional pathway for the reaction, not necessarily a pathway having a lower activation energy.Copper, Christine L.; Koubek, Edward. J. Chem. Educ.1999, 76, 1714.

Using CBL Technology and a Graphing Calculator To Teach the Kinetics of Consecutive First-Order ReactionsJosé E. Cortés-Figueroa and Deborah A. MooreThis work proposes a demonstration to introduce first-order reactions using the CBL system. It then presents the analysis of two consecutive first-order reactions. The values of the rate constants that govern each reaction's rate are determined using the graphing and statistical capabilities of a TI-83 calculator. Cortés-Figueroa, José E.; Moore, Deborah A. J. Chem. Educ.1999, 76, 635.

Kinetics |

Laboratory Computing / Interfacing |

Rate Law

Chemistry Time: Factors Affecting the Rate of a Chemical ReactionThis activity can be used to introduce a unit on chemical kinetics, but it is simple enough to be used in a discussion of chemical reactions or experimental methods/procedures during the first weeks of the semester. The activity involves reacting bicarbonate with acid, a reaction with practical applications in everyday life.J. Chem. Educ.1998, 75, 1120A.

Kinetics |

Rate Law

An Analogy to Help Students Understand Reaction OrdersCharles J. MarzzaccoThis article describes a simple analogy to help students understand the concept of the rate law for a chemical reaction. The analogy involves the mathematical relationships between various characteristics of a cube and the length of its edge. Charles J. Marzzacco. J. Chem. Educ.1998, 75, 482.

A Laboratory Experiment Investigating Different Aspects of Catalase Activity in an Inquiry - Based ApproachDoris R. Kimbrough, Mary Ann Magoun, Meg LangfurThe action of the enzyme catalase on aqueous hydrogen peroxide to generate oxygen gas is a well-established demonstration. Catalase is typically obtained by aqueous extraction of a potato, and the potato extract is mixed together with 3% hydrogen peroxide. The oxygen that is produced can be collected over water. Variations on the procedure can demonstrate the dependence of catalytic activity on temperature or the presence of inhibitors.Kimbrough, Doris R.; Magoun, Mary Ann; Langfur, Meg . J. Chem. Educ.1997, 74, 210.

Strategic Consequences from Errors in Raoult's Law PaperStephen J. HawkesThis article is an apology addressing errors in a previously published paper, "Raoult's Law is a Deception" and the new line of thinking that developed as a result of finding the errors. Hawkes, Stephen J. J. Chem. Educ.1996, 73, 41.

Raoult's Law Is a DeceptionHawkes, Stephen J.Argument that Raoult's law should be omitted from introductory chemistry courses because of limited applicability and usefulness at that level of study.Hawkes, Stephen J. J. Chem. Educ.1995, 72, 204.

Rate Law |

Aqueous Solution Chemistry

Pictorial Analogies XIII: Kinetics and MechanismFortman, John J.Pictorial analogies for first order kinetics, the effect of concentration and temperature on reaction rate, and the requirement for proper molecular orientation for reaction.Fortman, John J. J. Chem. Educ.1994, 71, 848.

Reaction dynamicsLacks, DanielSoftware that simulates collisions of an atom with a diatomic molecule, allowing students to set the initial conditions and the type of atom or molecule involved.Lacks, Daniel J. Chem. Educ.1992, 69, 1010.

Reactions |

Rate Law

Simple and inexpensive kinetics: A student laboratory experiment and demonstration Erwin, David K.Laboratory experimentation, as well as in-class demonstration, involving the study of chemical kinetics can be performed using this safe, simple, and inexpensive apparatus. This apparatus requires only that systems to be studied must produce a gaseous product that can displace water.Erwin, David K. J. Chem. Educ.1992, 69, 926.

Reduction of permanganate: A kinetics demonstration for general chemistrySteffel, Margaret J.Using the reduction of MnO4- to Mn2+ in aqueous solution to demonstrate the four factors that control reaction rates in solution: the natures of the reactants, concentrations of the reactants, temperature, and the presence of a catalyst.Steffel, Margaret J. J. Chem. Educ.1990, 67, 598.

Polarized light and rates of chemical reactionsWeir, John J.This experiment provides the opportunity to introduce the principles of reaction kinetics, polarized light, and the chemistry of optically active compounds; the rate of the acid-catalyzed hydrolysis of sucrose to glucose and fructose is determined.Weir, John J. J. Chem. Educ.1989, 66, 1035.

Rate Law |

Kinetics |

Chirality / Optical Activity |

Carboxylic Acids

Computer simulation of chemical equilibriumCullen, John F., Jr.108. The "Great Chemical Bead Game" requires no instruments and presents the concepts of equilibrium and kinetics more clearly than an experiment. [October and November Computer Series both inadvertently called number 107. Numbering restored by skipping 109 and calling January 1990 number 110.]Cullen, John F., Jr. J. Chem. Educ.1989, 66, 1023.

Analysis of kinetic data with a spreadsheet programHenderson, JohnAn article about spreadsheet templates that accept concentration versus time data for several runs of an experiment, determination of least-squares lines through data points for each run, and will allow the user to exclude points from the least-squares calculation.Henderson, John J. Chem. Educ.1988, 65, A150.

Change in concentration with timeUmland, Jean B.Shows how the rate of a reaction is fast at first and then gradually decreases to zero when one reactant has been used up.Umland, Jean B. J. Chem. Educ.1985, 62, 153.

Computer simulation of elementary chemical kinetics Nase, Martha L.; Seidman, Kurt44. Bits and pieces, 16. The authors have developed several computer programs that simulate chemical kinetics for elementary first and second order processes. These programs can be used to generate kinetic data that can then be analyzed by the student in a variety of ways.Nase, Martha L.; Seidman, Kurt J. Chem. Educ.1983, 60, 734.

Treat 'em to TchaikovskyWhitman, MarkThe author shares a demonstration that attracts great student attention. Students are highly successful when answering questions about the phenomenon in this demonstration on ensuing exams.Whitman, Mark J. Chem. Educ.1983, 60, 229.

What is the rate-limiting step of a multistep reaction?Murdoch, Joseph R.The purpose of this paper is to point out the circumstances where analogies can be used successfully and to develop a generalization which can be used for all reactions, including those with polymolecular steps.Murdoch, Joseph R. J. Chem. Educ.1981, 58, 32.

Safety in oxygen atmospheresKnight, Homer T.; Isenberg, NorbertA practical way to illustrate the influence of concentration on the rate of a chemical reaction is to show a simulated oxygen tent.Knight, Homer T.; Isenberg, Norbert J. Chem. Educ.1980, 57, 453.

The kinetics of runningLarsen, Russell D.The consideration of running as a rate process has several advantages for a student studying chemical kinetics for the first time.Larsen, Russell D. J. Chem. Educ.1979, 56, 651.

Reaction rates for a homogeneously catalyzed reactionNechamkin, Howard; Keller, Elhannan; Goodkin, JeromeThe reaction of KMnO4 with hydrogen in an acidic medium is an example of a homogeneously catalyzed reaction that can be performed by college freshmen.Nechamkin, Howard; Keller, Elhannan; Goodkin, Jerome J. Chem. Educ.1977, 54, 775.

Rate Law |

Kinetics |

Catalysis

Water dipping kinetics. A physical analog for chemical kineticsBirk, James P.; Gunter, S. KayPhysical analogs of zero-, first, and second-order kinetics using the volume of water transferred by a dipper oriented in different directions with respect to a basin of water.Birk, James P.; Gunter, S. Kay J. Chem. Educ.1977, 54, 557.

The definition of the rate of a chemical reactionCanagaratna, S. G.Most texts take it as obvious that the rate of a reaction may be defined in terms of changes in concentration; this definition is valid only if the reaction takes place without change of volume.Canagaratna, S. G. J. Chem. Educ.1973, 50, 200.

Pseudo first-order kineticsCorbett, John F.A kinetic study of second-order reactions under first-order conditions can yield accurate second-order rate constants provided an empirical allowance is made for the depletion of the reactant in excess.Corbett, John F. J. Chem. Educ.1972, 49, 663.

A study of the physical and chemical rates of CaCO3 dissolution in HClBassow, Herbert; Hamilton, Doug; Schneeberg, Ben; Stad, BenThe authors describe the experimental procedure and a discussion of results for a study of the physical and chemical rates of CaCO3 dissolution in HCl.Bassow, Herbert; Hamilton, Doug; Schneeberg, Ben; Stad, Ben J. Chem. Educ.1971, 48, 327.

Acids / Bases |

Kinetics |

Reactions |

Rate Law

MiscellaneousAlyea, Hubert N.These twelve overhead projection demonstrations include rates of reactions, clock reactions, the effect of temperature and the presence of a catalyst on the decomposition of hydrogen peroxide, the relationship between viscosity and temperature, equilibria, solubility product, and the common ion effect.Alyea, Hubert N. J. Chem. Educ.1970, 47, A437.

Sealed tube experimentsCampbell, J. A.Lists and briefly describes a large set of "sealed tube experiments," each of which requires less than five minutes to set-up and clean-up, requires less than five minutes to run, provides dramatic results observable by a large class, and illustrates important chemical concepts.Campbell, J. A. J. Chem. Educ.1970, 47, 273.

The law of mass actionBerline, Steven; Bricker, ClarkIt is the purpose of this paper to present a derivation of the Law of Mass Action that should have meaning and could be used at an elementary level.Berline, Steven; Bricker, Clark J. Chem. Educ.1969, 46, 499.

Equilibrium |

Rate Law |

Kinetics

From stoichiometry and rate law to mechanismEdwards, John O.; Greene, Edward F.; Ross, JohnExamines the rules used by chemists as guidelines in developing mechanisms from stoichiometric and rate law observations. Edwards, John O.; Greene, Edward F.; Ross, John J. Chem. Educ.1968, 45, 381.

Stoichiometry |

Rate Law |

Kinetics |

Mechanisms of Reactions |

Equilibrium |

Reactive Intermediates

The revolution in elementary kinetics and freshman chemistryWolfgang, RichardNew developments in kinetics so fundamentally affect our most elementary conception of chemical change that they must inevitably be reflected in beginning courses in chemistry; includes an outline for freshmen on elementary chemical dynamics.Wolfgang, Richard J. Chem. Educ.1968, 45, 359.

A kinetics experiment for first year chemistryShaefer, William P.The exchange of iodine atoms between organic and inorganic iodides serves as a kinetics experiment for first year chemistry.Shaefer, William P. J. Chem. Educ.1964, 41, 558.

Kinetics |

Isotopes |

Rate Law

The oxidation of iodide ion by persulfate ionMoews, P. C., Jr.; Petrucci, R. H.Presents the oxidation of iodide ion by persulfate ion as an ideal reaction to study as part of an experiment on kinetics.Moews, P. C., Jr.; Petrucci, R. H. J. Chem. Educ.1964, 41, 549.